Chapter 16: Problem 127
Predict the products and tell whether the following reaction will occur to any measurable extent: $$ \mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow $$
Short Answer
Expert verified
The reaction will not occur to any measurable extent.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Acetic Acid
Acetic acid, chemically represented as \( \mathrm{CH}_{3} \mathrm{COOH} \), is a commonly known weak acid found in vinegar. It is known for its characteristic pungent smell and is used extensively in the food industry. The term "weak acid" indicates that acetic acid does not fully dissociate in water. Instead, it partially ionizes, forming the acetate ion \( \mathrm{CH}_3\mathrm{COO}^- \) and hydrogen ion \( \mathrm{H}^+ \).
Acetic acid's behavior in solution is important in understanding its role in chemical reactions. Its inability to donate protons readily makes it less reactive compared to stronger acids. This weak ionization is crucial when predicting the outcome of reactions involving acetic acid, such as in the presence of ions like chloride \( \mathrm{Cl}^- \).
In chemistry, acetic acid serves as an excellent example of a substance where reactivity is dictated by its nature as a weak acid, affecting how it interacts with other substances.
Acetic acid's behavior in solution is important in understanding its role in chemical reactions. Its inability to donate protons readily makes it less reactive compared to stronger acids. This weak ionization is crucial when predicting the outcome of reactions involving acetic acid, such as in the presence of ions like chloride \( \mathrm{Cl}^- \).
In chemistry, acetic acid serves as an excellent example of a substance where reactivity is dictated by its nature as a weak acid, affecting how it interacts with other substances.
Chloride Ion
The chloride ion, represented by \( \mathrm{Cl}^- \), is a negatively charged ion commonly found in various compounds and dissolved salts. It is well known as a component of table salt (sodium chloride \( \mathrm{NaCl} \)) and exists freely in aqueous solutions.
In chemistry, chloride ions are considered weak bases. This classification aligns with their low tendency to accept protons from other substances in solution. Because of this weak basic nature, chloride ions generally do not engage in significant interactions with many acids, especially weak acids like acetic acid.
The relatively inert behavior of chloride ions in solution is an important consideration when predicting reaction outcomes. Their role in chemical reactions frequently involves acting as spectator ions, which do not participate in or significantly affect the equilibrium of an acid-base reaction.
In chemistry, chloride ions are considered weak bases. This classification aligns with their low tendency to accept protons from other substances in solution. Because of this weak basic nature, chloride ions generally do not engage in significant interactions with many acids, especially weak acids like acetic acid.
The relatively inert behavior of chloride ions in solution is an important consideration when predicting reaction outcomes. Their role in chemical reactions frequently involves acting as spectator ions, which do not participate in or significantly affect the equilibrium of an acid-base reaction.
Reaction Reactivity
Reactivity in chemical reactions is influenced by the nature of the reactants involved. Reactivity can be seen as the capability and willingness of substances to engage in chemical changes. The example of acetic acid and chloride ion illustrates a scenario where minimal reaction occurs due to the inherent characteristics of the substances.
Acetic acid, being a weak acid, does not readily give up its protons, and chloride ions, being weak bases, do not seek protons with vigor. This combination leads to a negligible reaction. To evaluate reactivity, understanding the strengths of the acids and bases involved is essential. Weak acids and bases tend to show low reactivity with each other, as their efforts to exchange protons do not significantly alter their original states.
Overall, reactivity is determined by the potential energy change and the stabilization of products that might arise from a reaction. In cases like the one with acetic acid and chloride ions, no new stable products form, indicating low reaction reactivity.
Acetic acid, being a weak acid, does not readily give up its protons, and chloride ions, being weak bases, do not seek protons with vigor. This combination leads to a negligible reaction. To evaluate reactivity, understanding the strengths of the acids and bases involved is essential. Weak acids and bases tend to show low reactivity with each other, as their efforts to exchange protons do not significantly alter their original states.
Overall, reactivity is determined by the potential energy change and the stabilization of products that might arise from a reaction. In cases like the one with acetic acid and chloride ions, no new stable products form, indicating low reaction reactivity.
Acid-Base Reaction
Acid-base reactions are chemical processes that involve the transfer of hydrogen ions \( \mathrm{H}^+ \) between reactant species. These reactions are fundamental to many processes in both industrial and natural settings. In an acid-base reaction, an acid donates a hydrogen ion to a base.
In the specific case of acetic acid and chloride ion in solution, one might initially consider a potential acid-base reaction involving the donation of a proton from acetic acid to the chloride ion. However, given that the chloride ion is a very weak base and acetic acid is a weak acid, this transfer does not occur to any significant extent. Instead, both reactants remain largely in their original form, with little to no progress toward product formation.
In summary, for a distinct acid-base reaction to take place, there must be a considerable difference in the strengths of the acids and bases involved, resulting in significant ion transfer and change in the system. With acetic acid and chloride ion, such a disparity in strength is absent, leading to negligible reaction.
In the specific case of acetic acid and chloride ion in solution, one might initially consider a potential acid-base reaction involving the donation of a proton from acetic acid to the chloride ion. However, given that the chloride ion is a very weak base and acetic acid is a weak acid, this transfer does not occur to any significant extent. Instead, both reactants remain largely in their original form, with little to no progress toward product formation.
In summary, for a distinct acid-base reaction to take place, there must be a considerable difference in the strengths of the acids and bases involved, resulting in significant ion transfer and change in the system. With acetic acid and chloride ion, such a disparity in strength is absent, leading to negligible reaction.
